Reactions of the Halide Ions (CIE A Level Chemistry)

• Halide ions can also act as reducing agents and donate electrons to another atom
• The halide ions themselves get oxidised and lose electrons
• The reducing power of the halide ions increases going down the group
• This trend can be explained by looking at the ionic radii of the halides’ ions

The diagram shows that going down the group the ionic radii of the halogens increases

• Going down the group, the halide ions become larger
• The outermost electrons get further away from the nucleus
• The outermost electrons also experience more shielding by inner electrons
• As a result of this, the outermost electrons are held less tightly to the positively charged nucleus
• Therefore, the halide ions lose electrons more easily going down the group and their reducing power increases

The reducing power of the halide ions increases going down the group

Silver ions & ammonia

• Halide ions can be identified in an unknown solution by dissolving the solution in nitric acid and then adding a silver nitrate solution followed by ammonia solution
• The halide ions will react with the silver nitrate solution as follows:

AgNO₃(aq) + X^-(aq) → AgX(s) + NO₃^-(aq)

Ag⁺(aq) + X^-(aq) → AgX(s)

• • X^- is the halide ion in both equations

• If the unknown solution contains halide ions, then a precipitate of the silver halide will be formed (AgX)

A silver halide precipitate is formed upon addition of silver nitrate solution to halide ion solution

• Dilute followed by concentrated ammonia is added to the silver halide solution to identify the halide ion
• If the precipitate dissolves in dilute ammonia the unknown halide is chloride
• If the precipitate does not dissolve in dilute but in concentrated ammonia the unknown halide is bromide
• If the precipitate does not dissolve in dilute nor concentrated ammonia the unknown halide is iodide

Silver chloride and silver bromide precipitates dissolve on addition of ammonia solution whereas silver iodide doesn’t

Reaction of halide ions with silver nitrate & ammonia solutions table

Concentrated sulfuric acid

• Chloride, bromide and iodide ions react with concentrated sulfuric acid to produce toxic gases
• These reactions should therefore be carried out in a fume cupboard
• The general reaction of the halide ions with concentrated sulfuric acid is:

H₂SO₄(l) + X^-(aq) → HX(g) + HSO₄^-(aq)

(general equation)

Where X^- is the halide ion

Reaction of chloride ions with concentrated sulfuric Acid

• Concentrated sulfuric acid is dropwise added to sodium chloride crystals to produce hydrogen chloride gas

Apparatus set up for the reaction of sodium chloride with concentrated sulfuric acid

• The reaction that takes place is:

H₂SO₄(l) + NaCl(s) → HCl(g) + NaHSO₄(s)      

• The HCl gas produces is seen as white fumes

Reaction of bromide ions with concentrated sulfuric acid

• The thermal stability of the hydrogen halides decreases down the group
• The reaction of sodium bromide and concentrated sulfuric acid is:

H₂SO₄(l) + NaBr(s) → HBr(g) + NaHSO₄(s)     

• The concentrated sulfuric acid oxidises HBr which decomposes into bromine and hydrogen gas and sulfuric acid itself is reduced to sulfur dioxide gas:

2HBr(g) + H₂SO₄(l) → Br₂(g) + SO₂(g) + 2H₂O(l)

• The bromine is seen as a reddish-brown gas

Reaction of iodide ions with concentrated sulfuric acid

• The reaction of sodium iodide and concentrated sulfuric acid is:

H₂SO₄ (l) + NaI (s) → HI (g) + NaHSO₄ (s)          

• Hydrogen iodide decomposes the easiest
• Sulfuric acid oxidises the hydrogen iodide to several extents:
• The concentrated sulfuric acid oxidises HI and is itself reduced to sulfur dioxide gas:

2HI (g) + H₂SO₄ (l) → I₂ (g) + SO₂ (g) + 2H₂O (l)

• Iodine is seen as a violet/purple vapour
• The concentrated sulfuric acid oxidises HI and is itself reduced to sulfur:

6HI (g) + H₂SO₄ (l) → 3I₂ (g) + S (s) + 4H₂O (l)

• Sulfur is seen as a yellow solid
• The concentrated sulfuric acid oxidises HI and is itself reduced to hydrogen sulfide:

8HI (g) + H₂SO₄ (l) → 4I₂ (g) + H₂S (s) + 4H₂O (l)

• Hydrogen sulfide has a strong smell of bad eggs

Halide ion reactions with concentrated sulfuric acid table